Answer:
The pH of the solution is 4.76
Explanation:
The concentration of the acetic acid and sodium acetate are 0.500 mole per liter each
The Kₐ of the acetic acid is 1.74 × 10⁻⁵
The concentration of the acetic acid CH₃COOH = 0.500 mole per liter = 0.5 M
The concentration of the sodium acetate (conjugate base) = NaCH₃COO = 0.500 mole per liter = 0.5 M
The dissociation constant, Kₐ, is given by the relation;
[tex]K_a = \dfrac{[H_3O^+][CH_3COO^-]}{[CH_3COOH]}[/tex]
Therefore, we have;
Kₐ × [CH₃COOH]/[CH₃COO⁻] = [H₃O⁺]
1.74×10⁻⁵×0.5/0.5 = 1.74 × 10⁻⁵
Therefore, [H₃O⁺] = 1.74 × 10⁻⁵
pH = -㏒₁₀(1.74×10⁻⁵) = 4.76
The pH of the solution = 4.76.
